Question

HEN

A 45.2 g sample of Nitrogen gas, N2, has a volume of 3,456mL and a
temperature of 25.0 °C. What is the pressure of the gas? *
F
O 1160 kPa
O 1.15 kPa
O 11.4 kPa
SES
EBRER
96.8 kPa

Answer 1

Pressure of the nitrogen gas is 2290 kPa.

Step-by-step explanation:

Using the ideal gas equation, we can find the pressure of the gas using the equation as,

PV = nRT

Where P is the pressure = ?

V is the volume = 3,456 ml = 3.456 L

n is the number of moles =
`$(given mass)/(molar mass)` =
`$(45.2g )/(14 g/mol)` = 3.2 mol

R is the gas constant = 0.08205 L atm K⁻¹ mol⁻¹

T is the temperature = 25 + 273 = 298 K

Now, rewriting the equation, we will get,

P =
`$(nRT)/(V)`

=
`$(3.2 * 0.08205* 298 K )/(3.456 L)`

= 22.6 atm

Now Pressure in 22.6 atm is converted as 2290 kPa.